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Aqa A Level Chemistry > Energetics > Flashcards

Energetics Flashcards

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1
Q

What is there usually when there a chemical reaction happens?

A

Change in energy

Enthalpy change

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2
Q

Define Enthalpy change

A

∆H (delta H) of the heat energy transferred in a reaction at constant pressure. The units of ∆H are kJ mol-1

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3
Q

Ho of Enthalpy change means

A

Ho of Enthalpy change

Substances were in standard states and measurement was made under standard conditions

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4
Q

Standard conditions for Enthalpy change are?

A

Standard conditions are 100kPa pressure
298K
Stated temperature
ΔH298

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5
Q

Describe exothermic

A

Give out energy

ΔH is negative

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6
Q

Describe endothermic

A

Takes in energy

ΔH is positive

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7
Q

Exothermic reactions are usually

A 
Oxidation e.g.
Combustion of a fuel like methane
CH4(g) + O2 (g)   →    CO2(g) + H2O(l)
ΔcH=-890 kJ mol-1
Oxidation of carbohydrates eg. C6H12O6 in respiration
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8
Q

Endothermic examples

A

Thermal decomposition of calcium carbonate
CaCO3(s)-> CaO(s) + CO2(g) ΔH=+178kJmol-1
Main reactions of photosynthesis

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9
Q

In exothermic reactions what Happens to temperature

A

Increase

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10
Q

In endothermic reactions what Happens to temperature

A

Decrease

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11
Q

What happens in bonds when a reaction happens?

A

Reactant bonds are broken and product bonds are formed

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12
Q

What do you need to break bonds?

A

Energy so bond breaking is endothermic ΔH is positive

Stronger bonds take more energy to break

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13
Q

What happens when bonds are formed?

A

Energy is released so bond making is exothermic ΔH if negative
Stronger bonds release more energy when they form

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14
Q

What’s Enthalpy change for a reaction

A

The overall sum of these two changes
If you need more energy bonds then released when bonds made ΔH if positive
If less ΔH is negative

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15
Q

How do you get mean enthalpies do?

A

Up in data books

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16
Q

What’s bond Enthalpy?

A

The energy required to break bonds

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17
Q

When you break the same type of bond does it always require the same amount of energy?

A

No the energy needed to beak a bond depends on the environment its in

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18
Q

What’s mean bond Enthalpy?

A

The average energy needed to break a certain type of bond over a range of compounds

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19
Q

Example of mean bond Enthalpy

A

Water has two O-H bonds
First bond Enthalpy= +492kJ mol-1
Second bond Enthalpy= +428kJmol-1
Mean bond Enthalpy 492+428/2=+460kJmol-1

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20
Q

Bond enthalpies are?

A

Always positive because breaking bonds is always endothermic

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21
Q

What happens in a chemical reaction during bond formation?

A

Energy absorbed to break bonds and given out during bond formation

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22
Q

Enthalpy change=

A

Enthalpy change=

Total energy absorbed-total energy released

23
Q

What is so because bond energies are averages?

A

Enthalpy changes aren’t exact

They are slightly less accurate than using Hess’s law

24
Q

Define standard Enthalpy of formation?

A

ΔfHo

Is the Enthalpy change when 1 mole of compound is formed from its elements in their standard states

25
Q

Define standard Enthalpy of combustion

A

ΔcHo is the Enthalpy change when one mole of a substance is completely burned in oxygen under standard conditions

26
Q

What can you find out using calorimetry?

A

Enthalpy change

27
Q

How can you use calorimetry to find out how much heat is given out by a reaction?

A

By measuring a temperature

28
Q

What do you use to find the enthalpy combustion of a flammable liquid? Step 1

A

You burn it inside a calorimeter?

29
Q

What do you use to find the enthalpy combustion of a flammable liquid? Step 2

A

As fuel burns it heats the water
You can work out heat energy that has been absorbed by water if you know the mass of water the temperature change and the specific heat capacity of water (4.18Jg-1K-1)

30
Q

What would ideally happen in calorimetry?

A

The heat given out by the fuel as it burns would be absorbed by the water allowing you to work out the enthalpy change of combustion exactly

31
Q

What actually happens in calorimetry?

A

You always lose some heat so hard to get really accurate result

32
Q

Formula to calculate enthalpy change from a calorimetry experiment?

A

q=mcΔT
Q= heat lost or gained in joules same as enthalpy change if pressure is constant
M= mass of water/ other solution in calorimeter (g)
C= specific heat capacity of water (4.18Jg-1K-1)
ΔT= change in temperature (K) of water/ solution

33
Q

What’s specific heat capacity of water?

A

The amount of heat energy it takes to raise the temperature of 1g by 1K

34
Q

The official ΔT units are K but what are they equal to for change in temperature?

A

oC

35
Q

In a laboratory experiment, 1.16g of an organic liquid fuel were completely burned in oxygen. The heat formed during the combustion raised the temperature ΔcHo of the fuel. Mr is 58.0
Step 1

A

Calculate amount of heat capacity using q=mcΔT

q= 100 x 4.18 x (358-295)= 26334J

36
Q

In a laboratory experiment, 1.16g of an organic liquid fuel were completely burned in oxygen. The heat formed during the combustion raised the temperature ΔcHo of the fuel. Mr is 58.0
Step 2

A

Standard enthalpies are always given in kJ mol-1

Change units of q from joules to kilojoules (26334/1000)= 26.334kJ

37
Q

In a laboratory experiment, 1.16g of an organic liquid fuel were completely burned in oxygen. The heat formed during the combustion raised the temperature ΔcHo of the fuel. Mr is 58.0
Step 3

A

Standard enthalpy of combustion is energy produced by burning 1 mole of fuel. So find out how many moles of girl produced this much energy using number of moles= mass/Mr
Number of moles of fuel= 1.16/ 58=0.0200

38
Q

In a laboratory experiment, 1.16g of an organic liquid fuel were completely burned in oxygen. The heat formed during the combustion raised the temperature ΔcHo of the fuel. Mr is 58.0
Step 4

A

Heat produced by 1 mole of fuel =-26.334/0.0200=-1316.7kJmol-1
-1320kJmol-1

39
Q

What can calorimetry also be used for?

A

Calculate enthalpy change for a reaction that happens in solution e.g. Neutralisation, dissolution (dissolving) or displacement

40
Q

How do you find the enthalpy for a neutralisation reaction?

A

Add known volume of acid to insulated container (e.g. Polystyrene cup) and measure the temperature
Add known volume of alkali and record temperature change (stir solution to make sure it’s evenly heated)
Work out heat needed to raise temperature of solution q=mcΔT this equals the heat given out by the reaction

41
Q

What happens if the alkali is solid?

A

Known mass

42
Q

What happens if you’re mixing two solutions?

A

Need to include masses of both

43
Q

What can you assume about all liquids?

A

Have same density as water since 1cm3 leg water has mass of 1g
E.g. 50cm3 of solution
Mass=50g for q=mcΔT

44
Q

What do you need to go if you are trying to find the energy change per mole of reactant?

A

Moles= concentration (mol dm-3) x volume(dm3)

To find number of moles of substance in a solution

45
Q

Experimental problems with all calorimetry?

A

Some heat will be absorbed by container rather than going towards heating up the water
Some heat always lost to surroundings during experiment (however well the containers insulated)

46
Q

Experimental problems that only apply to flammable liquid calorimetry?

A

Some combustion may be incomplete meaning less energy will be given out
Some flammable liquid may escape by evaporation (usually quite volatile)

47
Q

Hess’s law?

A

Total enthalpy change of a reaction is independent of the route taken

48
Q

What does ΔrH mean?

A

The enthalpy change of a reaction

49
Q

What’s Hess’s law good for?

A

Working out enthalpy changes that you can’t find directly by doing an experiment

50
Q

Enthalpy changes of formation are useful for?

A

Calculating enthalpy change you can’t find directly

51
Q

What do you need to know to use Hess’s law?

A

ΔfHo for all reactants and products that are compounds

ΔfHo for all elements is zero elements being formed from element so no change

52
Q

For formations ΔrHo?

A

The sum of ΔfHo (products) - the sum of ΔfHo (reactants)

If big 2 multiple by 2 to get sum

53
Q

What are standard enthalpy changes measured at?

A

298K

54
Q

What happens if you go backwards along an arrow in Hess’s law diagram?

A

Substraction enthalpy change that goes with that arrow

E.g. Could use ΔfHo for ethanol using these routes instead

Aqa A Level Chemistry (12 decks)

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